0
What else can I help you with?
How would you expect the extent of overlap of atomic orbitals to vary in the series FICl IBr I2 and?
The extent of overlap of atomic orbitals decreases from F2 to I2 in the series. This is due to an increase in the size of the atoms and therefore a larger distance between their nuclei, leading to weaker orbital overlap.
Is atomic radii of d block elements is smaller than p block reason out?
Yes, the atomic radii of d-block elements are generally smaller than p-block elements due to greater effective nuclear charge resulting from the filling of d orbitals that shield the outer electrons less effectively compared to p orbitals. This leads to stronger attraction between the nucleus and valence electrons, resulting in a smaller atomic size for d-block elements.
What does the term atomic radius mean?
Atomic radius is a measure of the size of an atom, typically defined as half the distance between the nuclei of two atoms of the same element that are bonded together. It represents the average distance from the nucleus to the outermost electron shell. Atomic radius generally decreases across a period on the periodic table and increases down a group.
How would the 4d orbitals differ from the 3d orbitals?
The 4d orbitals are larger in size and have higher energy levels compared to the 3d orbitals. They have more complex shapes due to the presence of an additional orbital shell, resulting in different spatial orientations and lobes. The 4d orbitals also have a larger number of nodes, which affects their electron density distribution.
What elements has the smallest atomic size K Ca Na Ar or Kr?
The element with the smallest atomic size is Argon (Ar) as it has the highest atomic number among the options given. Atomic size generally decreases from left to right across a period in the periodic table.
Why is the atomic size considered to have no definite boundary?
Atomic size is defined as the distance between the nucleus and the outermost electron in an atom. Since electrons occupy regions of space called orbitals, which have fuzzy boundaries, it is difficult to pinpoint an exact boundary of an atom. Additionally, the electron cloud distribution is not uniform, making the atomic size less precise.
How does the size of an atomic nucleus compare with the size of the whole atom?
Think of the sun as the nucleus and the oort cloud (past pluto) as where the electron orbitals start. The size (volume) of the nucleus is tiny compared to the size (volume) of the atom (defined by the extent of the electron cloud).
What meant by hybridization of atomic orbital?
Hybridization of atomic orbitals is the intermixing of atomic orbitals having a approximate energy to form equal number of hybrid orbitals having the same shape, size and energy but pointing in different directions. The new orbitals which are formed are "hybrids" of the originals and have properties that are somewhere in between. For example, a common hybridization is sp3 where three p orbitals combine with an s orbital to form four new orbitals. Other combinations (such as sp and sp2) are also possible.
How are two blank pages of the exact shape and size different?
At an atomic level they cannot be exactly the same shape or size.
How would you expect the extent of overlap of atomic orbitals to vary in the series FICl IBr I2 and?
The extent of overlap of atomic orbitals decreases from F2 to I2 in the series. This is due to an increase in the size of the atoms and therefore a larger distance between their nuclei, leading to weaker orbital overlap.
Why element mercury liquid at room temperature?
the metallic bonding is not very stong among the atoms due to larger atomic size and full filled 'd' orbitals in Hg....
Are all s orbitals the same size?
Yes, all s orbitals have the same size, regardless of the energy level they are in. This is because s orbitals are spherical in shape with the electron density focused around the nucleus.
Why the size of atom does not decrease regularly in a period?
pagal u tell
Which has smaller atomic size helium or fluorine or neon?
He has the smaller atomic size. Fluorine has the larger atomic size from these 3. He is a noble gas.
What is the effect of an additional electron have on atomic size?
According to me the atomic size of an atom increases or decreses with the change in the number of shells. As atomic size is defined as the distance between the nucleus and valence shell of an atom. So, the addition of an electron does not effect the atomic size. As we can see in the periodic table that while moving along a group the number of electrons increases along with increase in no. of shells, while the atomic size tends to be increase with addition of shells and neglecting the addition of electrons. Same is the case while moving along a period. Atomic size decreases while the attraction between increased nuleus charge increases . Thus the size of the atom decreases.
What has the smallest radius for rb k k rb?
In the context of atomic physics, the smallest radius for an atomic orbital is typically found in the hydrogen atom, where the radius is defined by the Bohr model. For the ground state (n=1), the Bohr radius is approximately 0.529 angstroms. In multi-electron atoms, the effective nuclear charge and electron-electron interactions can influence the size of the orbitals, but for a hydrogen-like atom (one electron), the smallest radius occurs at n=1.
Why OF6 compound is not known?
For the formation of this compound there should be six unpaired electrons in oxygen atom and this is not possible due to absence of 'd' orbitals , secondly the small atomic size of oxygen can not accommodates six fluorine atoms.
